To do so, we need to identify the change in oxidation state for each element in the reaction.
Recall the mnemonic for redox reactions:
Loss Electrons → Oxidation → Reducing Agent
Gain Electrons → Reduction → Oxidizing Agent
Reaction: 2 NO(g) + O2(g) → 2 NO2(g)
This is neither a peroxide nor superoxide, which means O.S. of O = –2.
This is also a neutral compound so the total oxidation state is zero.
O.S. of N + O.S. of O = 0
O.S. of N + (–2) = 0
O.S. of N = +2
This is an atom in its elemental form, which means O.S. of O = 0.
You may want to reference (Pages 145 - 148) Section 4.5 while completing this problem.
The commercial production of nitric acid involves the following chemical reactions:
In the following redox reaction identify the element undergoing oxidation and the element undergoing reduction.
2 NO(g) + O2(g) → 2 NO2(g)
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